A) \[{{3170}^{o}}C\]
B) \[\underset{chloropropane}{\mathop{C{{H}_{3}}C{{H}_{2}}C{{H}_{2}}Cl}}\,\xrightarrow[-KCl;-{{H}_{2}}O]{Alc.\,KOH}\underset{\Pr opene}{\mathop{C{{H}_{3}}CH=C{{H}_{2}}}}\,\]
C) \[\xrightarrow{B{{F}_{3}}/THF}{{(C{{H}_{3}}C{{H}_{2}}C{{H}_{2}})}_{3}}B\]
D) \[\xrightarrow{C{{H}_{3}}COOH}\underset{propane}{\mathop{C{{H}_{3}}C{{H}_{2}}C{{H}_{3}}}}\,\]
Correct Answer: C
Solution :
The reaction of oxidation of ferrous oxalate by potassium dichromate in acidic medium is written as \[\Delta {{G}^{o}}=3\Delta G_{f}^{o}(C{{O}_{2}})-2\Delta G_{f}^{o}(A{{l}_{2}}O{{ & }^{3}})\] \[=3(-394)-2(-1520)\] \[=1858kJ\] 2 moles of \[\Delta {{G}^{o}}=-nFE_{cell}^{o}\] are oxidised by = 1 mole of \[-E_{cell}^{o}=\frac{1858\times 1000}{12\times 96500}=1.60V\] \[\gamma -H\] 1 mole of FeC204 will be oxidised by \[\alpha \] mole of \[FeS{{O}_{4}},\]
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